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Chemical Equations and Reactions

Explore the characteristics of chemical reactions, indications of change, and learn to balance equations effectively. Practice with sample problems and demonstrations showing reactions like copper with nitric acid. Enhance your knowledge of diatomic elements and the law of conservation of mass.

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Chemical Equations and Reactions

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  1. Chemical Equations and Reactions Mrs. Taylor Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  2. Oh, That Curious Ira Remsen! 1846-1927 Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  3. Demonstration Demonstration Ira Remsen DemoCu (s) + HNO3(aq)  CuNO3 (aq) + H2(g) Chemical Reactionshttp://www.metacafe.com/watch/650550/nitric_acid_acts_upon_a_copper_penny_experiment/ Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  4. Indications of a Chemical Reaction Proof: one or more substances has changed identity – chemical change • Evolution of energy as heat and/or light • Production of a gas • Formation of a precipitate • Color change Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  5. Demonstration Demonstration Red, White and Blue Reactionhttp://www.chem.ox.ac.uk/vrchemistry/FilmStudio/redwhiteblue/page01.htm Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  6. Indications of a Reaction Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  7. Characteristics of a Chemical Reaction • The equation must contain the correct formulas for the reactants and products. • Diatomic elements: I2 Br2 Cl2 F2 O2 N2 H2 • The law of conservation of mass must be satisfied. (Mass cannot be created or destroyed) • Coefficients – a whole number that appears in front of a formula in a chemical equation. Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  8. Diatomic Elements p. 263 Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  9. Additional Symbols p. 226 Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  10. Additional Symbols p. 226 Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  11. Balancing Chemical Equations RULES OF THE GAME: Only coefficients can be added or changed. Once formulas are written subscripts can not be changed. Balance polyatomic ions that appear on both sides as a single unit. Balance H and O last. Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  12. Practice ___H2 + ____N2 → ____NH3 ____NaClO3 → ____NaCl + ____O2 ___Al2(SO4)3 + ___Ca(OH)2 → ____Al(OH)3 + ____CaSO4 ____C2H6 + ____O2 → ____CO2 + ____H2O Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  13. Sample Problem p.272 The reaction of zinc with aqueous hydrochloric acid produces a solution of zinc chloride and hydrogen gas. Write a balanced equation for the reaction Insert Holt Chemistry Visualizing Matter Disc 1 Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

  14. BALANCE THE EQUATIONS ____Al + ____N2 → ____AlN ____Fe + ____O2 → ____Fe3O4 ____ZnS + ____O2 → ____ZnO + ____SO2 ____Na + ____H2O → ____H2 + ____NaOH Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

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